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Chemistry > Unit 1: What is Matter? > Flashcards

Unit 1: What is Matter? Flashcards

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1
Q

Solid to Liquid

A

Melting

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2
Q

Liquid to Solid

A

Freezing

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3
Q

Solid to Gas

A

Sublimation

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4
Q

Gas to Solid

A

Deposition

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5
Q

Gas to Liquid

A

Condensation

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6
Q

Liquid to Gas

A

Vaporization

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7
Q

Define matter

A

Any substance that has mass and takes up space by having volume

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8
Q

What does the amount of energy needed to change states depend on?

A

It depends on the strength of forces between the particles of the substance

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9
Q

What happens to the melting and boiling point of a substance when the forces between the particles are stronger?

A

The stronger the forces between the particles, the higher the melting point and boiling point of the substance because more energy is needed to separate them.

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10
Q

Explain what happens to particles during changes of state

A

The closeness, arrangement and motion of the particles in a substance change when it changes state.

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11
Q

In which state are the particles randomly arranged?

A

Particles are randomly arranged in liquids and gases.

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12
Q

In which state are the particles only able to vibrate in a fixed position?

A

Particles in solids can only vibrate in a fixed position.

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13
Q

Which state can be compressed or squashed easily?

A

A gas can be compressed or squashed easily

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14
Q

Which state cannot flow from place to place?

A

Solids cannot flow from place to place

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15
Q

Particles in which state have no bonds?

A

Particles in gases have no bonds

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16
Q

Particles in which state sit in a regular pattern and are held together tightly by bonds?

A

Particles in solids sit in a regular pattern and are held together tightly by bonds

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17
Q

What happened to the pressure of gases when it is heated at constant volume?

A

When the temperature of a gas is increased, its pressure increases.

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18
Q

State what occurs when enough thermal energy is applied.

A

Boiling

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19
Q

Outline what a change of state is known as.

A

A physical change of a substance from one state to another.

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20
Q

Define density.

A

The degree of compactness of a substance

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21
Q

What is the density formula

A

Density = mass/volume

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22
Q

An object has a mass of 570 g and a volume of 2280 cm3. Calculate its density.

A

Density = 570 / 2280 = 0.25/cm3

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23
Q

A cat has volume 0.004 m3 and density 980 kg/m3. Calculate the mass of the cat.

A

980 x 0.004 = 3.92kg

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24
Q

A bottle of water has a density of 1000 kg/m3 and mass of 0.5 kg. Calculate the volume of the water bottle giving your answer in litres.

A

Volume = 0.5 / 1000 = 0.0005m3

0.0005 x 1000 = 0.5L

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25
Q

Identify the difference between atoms, elements, compounds & mixtures in terms of physical & chemical properties.

A

Elements contain only one type of atom.

Compounds contain two or more types of atoms that are chemically bonded.

Mixtures are two or more different types of atoms that are not chemically bonded.

An Atoms is the smaller particle of matter comprising an element.

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26
Q

List signs that a chemical reaction has taken place

A

Increase or decreases in temperature
Colour change
Formation of a gas (bubbles)
Change in properties (boiling point, melting point, smell, taste, density, texture, etc.)

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27
Q

List signs that a physical reaction has taken place

A

Change in size or shape.
Change in state of matter.
Reversible.
No new substance formed

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28
Q

Iron (grey) reacts with sulfur (yellow) when heated to produce black iron sulfide, state whether this is a chemical or physical change?

A

Chemical Change

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29
Q

Describe the properties of solids in terms of the volume, shape, arrangements, closeness and motion of particles.

A

A Solid is a substance that has a fixed shape and a fixed volume.

Solid particles have regular arrangements and are stable.

They are very close together and have vibrating movements.

Molecules of solid-state are capable of vibrational motion due to strong intermolecular forces. In vibrational motion, molecules move back and forth.

However, by decreasing the temperature ‘melting’, the particles would have less energy that changes the state from solid to liquid.

30
Q

Describe the properties of liquids in terms of the volume, shape, arrangements, closeness and motion of particles.

A

A liquid has a fixed volume but not a fixed shape.

It doesn’t have a regular arrangement as it is quite disordered.

They are slightly further apart and change positions with frequent collisions.

Liquid particles take the shape of the container.

Liquids have more kinetic energy than solids.

Liquids have show rotational motion as the molecule rotates in space due to weak intermolecular forces.

By decreasing the temperature ‘evaporation’, particles would have less energy which would cause it to break bonds and change states from liquid to gas.

31
Q

Describe the properties of gases in terms of the volume, shape, arrangements, closeness and motion of particles.

A

Particles fill up the container.

They don’t have regular arrangements as they are totally randomly arranged.

They are very far apart and fast moving with occasional collisions.

A gas can be compressed into very small spaces.

Gases have translational motion as the molecules move in certain directions because they have too much energy to remain attached to each other.

Gases have more kinetic energy than liquids.

By increasing the temperature ‘condensing’ the particles would have more energy that would cause the change from gas to liquid. By increasing the temperature of the liquid ‘freezing’ particles would have more energy that would cause them to change from liquid to solid.

32
Q

What happens to a substance when it increases in temperature?

A

When a substance increases in temperature, heat is being added, and its particles are gaining kinetic energy.

33
Q

Why solids have a fixed shape?

A

Solids have a fixed shape because the particles are tightly packed and cannot move around.

34
Q

Why a gas can be easily squashed?

A

A gas can be easily squashed because there is space between the particles.

35
Q

Why a liquid can be easily poured?

A

A liquid can be easily poured because it takes the shape of the container.

36
Q

Define the law of the conservation of mass

A

The law of conservation of mass states that mass in an isolated system is neither created nor destroyed by chemical reactions or physical transformations.

According to the law of conservation of mass, the mass of the products in a chemical reaction must equal the mass of the reactants.

37
Q

Describe the spacing of particles in solid, liquid and gas.

A

Solid: very close together
Liquid: slightly further apart
Gas: Very far apart

38
Q

Describe the arrangement of particles in solid, liquid and gas.

A

Solid: regularly arranged
Liquid: quite disordered
Gas: totally randomly arranged

39
Q

Describe the movement of particles in solid, liquid and gas.

A

Solid: vibrating
Liquid: changing positions with frequent collisions
Gas: fast moving with occasional collisions

40
Q

Explain the difference between pure and impure substances

A

A substance made out of only one kind of particle and has a fixed or constant structure.
A substance made out of two or more kinds of particles and doesn’t have a fixed or constant structure.

41
Q

What name is given to a substance that contains two types of atom that are not chemically joined together?

A

When two substances are mixed but not chemically joined to each other, they form a mixture.

42
Q

What process allows you to smell freshly baked bread in a supermarket, even when you are far from the bakery aisle?

A

Diffusion allows the smell particles to spread through the air and reach your nose.

43
Q

Deduce the factors that affect the movement of the particle

A

Temperature: At higher temperature, particles move faster.

Concentration gradient: can influence how much, how fast particles move.

44
Q

Describe particle movement as translational, vibrations and rotations.

A

Molecules of solid-state are capable of vibrational motion due to strong intermolecular forces. In vibrational motion, molecules move back and forth.

Liquids have show rotational motion as the molecule rotates in space due to weak intermolecular forces.

Gases have translational motion as the molecules move in certain directions because they have too much energy to remain attached to each other.

45
Q

Define the term diffusion

A

The net movement of gas or liquid particles from an area of high concentration to an area of lower concentration.

46
Q

Describe the dependence of rate of diffusion of molecular mass

A

The lower molecular mass, the faster a gas will diffuse because the light particles bounce further than the heavier ones after it collides with other particles.

47
Q

Explain factors that affect the rate of diffusion

A

Temperature: As the temperature increases, the kinetic energy associated with each particle increases. As a result of this, particles will move faster. If they can move faster, they can also diffuse faster. Therefore, the rate of diffusion increases.

Mass of particle: Heavier particles will move more slowly and so will have a slower rate of diffusion. As the mass of particle decreases, there will be smaller particles that will diffuse faster because they can move faster.

Density and viscosity: If the medium that a given particle has to diffuse through is less dense or less viscous, then the particles will be able to move more quickly and will diffuse faster

Concentration: If the difference in concentration is higher, then the molecules will go down the concentration gradient faster and the rate of diffusion will increase.

48
Q

Deduce factors that affect pressure

A

Heat: If there are hot gas, there are more collisions that are more energetic and more collisions means more pressure so therefore, the pressure increases.

Concentration: the higher concentration, the more particles collide and bump into each other and more collisions means more pressure so therefore, the pressure increases.

49
Q

Investigate Brownian motion

A

He found that any fine particle suspended in water executes a similar random motion.

50
Q

Outline the state(s) of matter in which particles are constantly moving?

A

When the temperature increases in the substance, the particles have more kinetic energy and are constantly moving. In gases, particles are constantly moving.

51
Q

State the type of property when a silver spoon begins to tarnish?

A

When a silver spoon begins to tarnish it forms a new substance that can’t be reversed, it also affects the substances involved in the change and thus it’s a chemical change.

52
Q

Describe what will happen to the candle overtime and make reference to the type of change for the wick and wax?

A

the wick will burn and produce ash, it is not reversible, so a new substance is formed as a result, it is a chemical change. The wax will result in melting, which the particles will then rearrange, this means that it is reversible and therefore, I believe that it is a physical change.

53
Q

Magnetism, solubility and malleability are physical properties of matter. Explain how these properties differ from chemical properties.

A

In a physical property the particles are rearranged which is reversible. On the other hand, in a chemical property the substances react to form new substances which cannot be reversed.

54
Q

Alisa placed a small seashell on the pan of a balance. State the other tool she needs to calculate the density of the seashell?

A

She needs a graduated cylinder to calculate the density

55
Q

State which of the following is a pure substance or impure substance: Element, compounds, mixtures?

A

Element & compound: pure

Mixture: impure

56
Q

Calculate the weight of the ethyl alcohol that exactly fills a 200.0 mL container? The density of ethyl alcohol is 0.789 g/mL.

A

g = (0.789 g/mL) (200.0 mL) = 158g

57
Q

A block of lead has dimensions of 4.50 cm by 5.20 cm by 6.00 cm. The block weighs 1587 g. From this information, calculate the density of lead. Write your answer in 2 significant figures and then into scientific notation.

A

g = (0.8765 g/mL) (250.0 mL) = 219.1 g

58
Q

28.5 g of iron shot is added to a graduated cylinder containing 45.50 mL of water. The water level rises to the 49.10 mL mark, From this information, calculate the density of iron.

A

49.10 – 45.0 = 3.6 38.5/3.6 = 7/9g/mL

59
Q

Scientists conduct experiment under standard conditions for temperature and pressure, state the temperature (K) and pressure (atm) used?

A

STP: 0 degrees Celsius and 1atm

60
Q

Explain why a balloon filled with helium gas will deflate faster than a balloon filled with air.

A

Gases, such as the air or helium inside a balloon, take the shape of the sealed container they are in. They spread out by diffusion so that the space is filled up evenly with gas molecules. They move in a straight line until they collide with another gas molecule or hit the container’s wall, and then they rebound and continue in another direction until they hit another gas molecule or the balloon. An increase in temperature will increase the average kinetic energy of the gas molecules. This means they move faster and have more frequent and harder collisions inside the balloon. The pressure on the balloon is increased and it expands.

61
Q

What are the three states of matter?

A

Solid, liquid, and gas

62
Q

How can the state of matter of a substance be identified?

A

The state of matter of a substance can be identified by the motion of the particles and the distance between them

63
Q

What is the kinetic theory?

A

The kinetic theory explains that gas pressure was the result of millions of tiny collisions between ball-like particles

64
Q

What is the kinetic molecular theory?

A

The kinetic molecular theory is the theory that explains the physical properties of matters and changes of state in terms of the movement and arrangement of their constituent particles

65
Q

What is a compound?

A

A compound is a substance made of two or more elements that are chemically bonded. A compound is a pure substance.

66
Q

Define enthalpy of fusion / latent heat of fusion

A

The energy required to melt one-unit measurement of a substance from solid to liquid

67
Q

In which state of matter is water densest?

A

Water particles are densest in their liquid state.

68
Q

Define enthalpy of vaporization / latent heat of vaporization

A

The energy required to evaporate one-unit measurement of a substance from liquid to gas

69
Q

Why does the temperature of a liquid not go overs its boiling point when heated?

A

When a substance is being heated, the temperature of the substance does not change because all the thermal energy is going into breaking the intermolecular forces.

70
Q

Which state change processes are exothermic?

A

Freezing, condensation, and deposition

71
Q

Which state change processes are exothermic

A

Melting, vaporization. and sublimation

Chemistry (12 decks)

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